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Question 1

Electron cloud

Answer 1

Consists of high energy electrons existing in energy shells

Question 2

Ion

Answer 2

A charged particle that is formed when an atoms gains or loses electrons from its outer shell

Question 3

1s² 2s² 2p⁶ 3s¹

What do the 1, 2 and 3 Infront mean

Answer 3

Shell Number

Question 4

1s² 2s² 2p⁶ 3s¹

What do the s and p’s mean

Answer 4

Subshell that is being filled

Question 5

1s² 2s² 2p⁶ 3s¹
What do the ² ⁶ ¹

Answer 5

Number of electrons in subshell

Question 6

Hund’s Rule

Answer 6

Every Orbital in a subshell is singly occupied being any orbital is doubly occupied

Question 7

Shell vs subshell vs orbital

Answer 7

Shells are broad energy levels.

Subshells are divisions within shells that group orbitals of similar energy.

Orbitals are specific regions in a subshell where electrons exist.

Question 8

How many electrons can orbitals hold

Answer 8

2

Question 9

Number of orbitals in s-subshell

Answer 9

1

Question 10

Number of orbitals in p-subshell

Answer 10

3

Question 11

Number of orbitals in d-subshell

Answer 11

5

Question 12

Number of orbitals in f-subshell

Answer 12

7

Question 13

What is the maximum number of electrons in a shell

Answer 13

2𝑛²

Question 14

Shells

Answer 14

Shells:

Shells are the major energy levels in an atom.

They are represented by the principal quantum number 𝑛 (e.g., 𝑛 = 1, 2, 3 etc)

The maximum number of electrons a shell can hold is determined by the formula 2𝑛²

Question 15

Subshells

Answer 15

Each shell is divided into subshells of similar energy.

Subshells are labeled s, p, d, and f.

Each type of subshell has a different maximum number of electrons:

s-subshell: 2 electrons

p-subshell: 6 electrons

d-subshell: 10 electrons

f-subshell: 14 electrons

Question 16

Orbitals

Answer 16

Orbitals are the regions within a subshell where electrons are most likely to be found.

Each orbital can hold a maximum of two electrons.

The number of orbitals in each subshell is as follows:

s-subshell: 1 orbital (holds 2 electrons)

p-subshell: 3 orbitals (each holding 2 electrons, total 6)

d-subshell: 5 orbitals (each holding 2 electrons, total 10)

f-subshell: 7 orbitals (each holding 2 electrons, total 14)

Question 17

Anion

Answer 17

Negative ion formed when non-metal atoms gain electrons to match the number of valence e⁻ of their nearest noble gas.

Question 18

Cation:

Answer 18

positive ion formed when metal atoms lose e⁻ to match the number of valence e⁻ of their nearest noble gas.

Question 19

Diatomic molecules:

Answer 19

where two atoms of the same element share e⁻.

Question 20

Ion

Answer 20

A charged particle

Question 21

Polyatomic ion

Answer 21

A polyatomic ion is an ion composed of two or more atoms that are covalently bonded and function as a single charged entity.

Question 22

Equation of Cation for H

Answer 22

H -> H⁺ + e⁻

Question 23

Equation of Anion for F

Answer 23

F + e⁻ -> F⁻

Question 24

Naming of ionic compounds

Answer 24

Metal followed by non-metal
no extra prefixes
Metal -> Original name
Non - metal -> “-ide” suffix

Question 25

What is a dipole

Answer 25

A dipole is the separation of charge in a molecule due to differences in electronegativity. One end becomes partially positive (δ⁺), and the other partially negative (δ⁻). Types: Permanent Dipole: Found in polar molecules (e.g., HCl, H₂O). Instantaneous/Induced Dipole: Temporary charge shifts (e.g., London dispersion forces).

Question 25

Naming of Covalent compounds

Answer 25

First non-metal has original name, 2nd ends in "__ide" Prefixes Mono - (Only for 2nd non metal) Di Tri Tetra Penta Hexa Hepta Oct Non Dec

Question 26

Polar bonds in covalant compounds

Answer 26

If the electronegativities of the two atoms are very different, than the electron pair will tend toward the more negative of the two atoms

Question 27

Non-polar bonds in covalent compounds

Answer 27

Occurs between two atoms that are the same or have similar electronegativity

Question 28

Covalent network solids

Answer 28

Some elements mainly ( C and Si) Some elements (mainly C & Si) can form 4 covalent bonds with other elements (C & Si) to create a network (lattice) solid. These networks are very strong & hard have very high melting points Do not conduct electricity

Question 29

What does metals being malleable and ductile tell you about their structure

Answer 29

The attraction forces between the particles must be stronger than the repulsive forces when the layers are moved

Question 30

How to represent isotopes

Answer 30

Nuclear Notation (or Standard Isotopic Notation) → ᴬX Example: ¹⁴C (Carbon-14) Hyphen Notation - X-A Example: Carbon-14

Question 31

How does mass spectroscopy work

Answer 31

1: Sample is vaporized 2: Ion accelerated through electric field 3: Fast moving ions separated by a magnetic field

Question 32

Graph of Mass spectrometer: What the number of peaks tells us: What the position of peaks tells us: What the height of peaks tells us:

Answer 32

Number of isotopes Relative isotopic mass Relative abundance of the isotope (in comparison to other isotopes of that element)

Question 33

What is m / z

Answer 33

m/z (mass-to-charge ratio) is the ratio of an ion’s mass (𝑚) to its charge (𝑧). It determines the position of peaks in a mass spectrum and helps identify molecules.